Answer:
5Fe⁺² + MnO₄⁻ + 8H⁺ => 5Fe⁺³ + Mn⁺² + 4H₂O
Explanation:
Fe⁺² + MnO₄⁻ + H⁺ => Mn⁺² + Fe⁺³ + H₂O
5(Fe⁺² => Fe⁺³ + 1e⁻) => 5Fe⁺² => 5Fe⁺³ + 5e⁻
<u>MnO₄⁻ + 5e⁻ => Mn⁺² => MnO₄⁻ + 8H⁺ + 5e⁻ => Mn⁺² + 4H₂O</u>
=> 5Fe⁺² + MnO₄⁻ + 8H⁺ => 5Fe⁺³ + Mn⁺² + 4H₂O
the molarity of a solution made by dissolving 5.67 g of potassium chloride in enough water to make 100.0 mL of solution.
Answer:
The transition-metal have the highest oxidation number is Mo in Rb₃[MoO₃F₃]
Explanation:
Transition metals are metals that are found in the middle of the periodic table.
For the compounds:
Rb₃[MoO₃F₃]: Rb is an alkali metal that has a charge of +1. that means [MoO₃F₃] is -3. The oxyfluoride O₃F₃ has a charge of -9. That means the <em>Mo is +6</em>
K₄[Mn(CN)₆]: Potassium is +1, thus, the [Mn(CN)₆] is -4, As the CN is -1 and there are 6, the <em>Mn is +2</em>
Na[Ag(CN)₂]: As Na is +1, the [Ag(CN)₂] is -1. As CN are -1, the <em>Ag is +1</em>
K₂[PtCl₆]: Potassium is +1, the [PtCl₆] is -2, As the Cl are -1, the <em>Pt is +4</em>
[Co(NH₃)₄Cl₂]: The NH₃ are neutral, The Cl are -1, that means the <em>Co is +2.</em>
The transition-metal have the highest oxidation number is<em> Mo +6</em>
I hope it helps!
Answer:
MgBr₂
Explanation:
Here we need to find the molar proportions of the two elements which will give us the empirical formula of the compound. To do that,we need to determine the number of moles the grams given represent, and then convert them to whole numbers to find their proportions.
Atomic weght Br = 79.904 g/mol mol
⇒ mol Br = 32.0 g/ 79.904 g/mol = 0.40 mol
Atomic weight Mg = 24.305 g/mol
⇒ mol Mg = 4.9 g/24.305 g/mol = 0.20 mol
Their proportions are
0.40 Br ÷ 0.20 Mg = 2 Br ÷ 1 Mg
Empirical formula = MgBr₂